Coupled alkali-feldspar dissolution and secondary mineral precipitation in batch systems: 1. New experiments at 200 °C and 300 bars
Introduction
Silicate mineral dissolution and secondary mineral precipitation are integrated processes in chemical weathering and hydrothermal alteration of rocks. Numerous experiments have been conducted for measuring silicate mineral dissolution rates (Busenburg and Clemency, 1976, Holdren and Berner, 1979, Chou and Wollast, 1985, Knauss and Wolery, 1986, Nagy et al., 1991, Nagy and Lasaga, 1992, Burch et al., 1993, Gautier et al., 1994, Hellmann, 1994, Oelkers et al., 1994, Hellmann, 1995, Nagy, 1995, Stillings and Brantley, 1995, Brantley and Stillings, 1996). The primary focus of many of these studies, however, was to derive mineral dissolution rates from steady state chemical conditions. In such experiments, silicate minerals, mostly feldspars, are dissolved far from equilibrium and secondary mineral precipitation is avoided by adjusting the chemistry and rate of recirculation of the fluid phase. Results of these experiments have been enormously successful, providing a wealth of data on the rate and mechanism of mineral dissolution processes under a wide range of chemical and physical conditions.
Batch reactor experiments of feldspar hydrolysis, on the other hand, provide a different set of data, which address the broader context of congruency and incongruency, phase relations, mineral metastability, and interconnections between dissolution and precipitation reactions. Tremendous progress in our understanding of feldspar hydrolysis in closed systems has come from the seminal work by Helgeson and co-workers (Helgeson, 1968, Helgeson et al., 1969Helgeson et al., 1970, Helgeson, 1971, Helgeson, 1972, Helgeson, 1974, Helgeson, 1979, Helgeson et al., 1984). While the first feldspar hydrolysis experiments conducted in batch reactors provided valuable information on the mechanism of feldspar dissolution, as summarized in Helgeson (1971) and Petrovic (1976), technological development of experimental design and apparatus has allowed the sampling of fluid co-existing with minerals at a wide range of temperatures and pressures (Seyfried et al., 1987). Furthermore, electron microscopy and surface analytical techniques have advanced significantly, which allow more accurate identification of secondary minerals, even when such phases exist on the nanometer size scale (Penn et al., 2001, Zhu et al., 2006).
Here we report results of alkali-feldspar dissolution experiments in well-mixed batch reactors that were performed at 200 °C and 300 bars in order to examine mineral dissolution and precipitation processes in moderately acidic fluids. Although dissolution reactions of single feldspars have been reported in the literature (Busenburg and Clemency, 1976, Holdren and Berner, 1979, Helgeson et al., 1984, Chou and Wollast, 1985, Knauss and Wolery, 1986, Wollast and Chou, 1992, Gautier et al., 1994, Hellmann, 1994, Oelkers et al., 1994, Hellmann, 1995, Stillings and Brantley, 1995, Brantley and Stillings, 1996, Hellmann and Tisserand, 2006), only a few experimental studies have been performed on feldspars with complex compositions (Morey and Fournier, 1961, Lagache, 1976, Rafal'skiy et al., 1990, Tsuchiya et al., 1995). The combination of time series monitoring of fluid chemistry and mineral analysis (scanning electron microscopy (SEM), high resolution transmission electron microscopy (HRTEM), X-ray diffraction (XRD), X-ray photoelectron spectroscopy (XPS), and electron microprobe analysis (EMPA)) at different reaction stages represents an insightful experimental strategy to assess geochemical controls on the temporal evolution of minerals and coexisting fluids. While this approach is relevant to mass transfer processes in a variety of natural and engineered hydrologic and hydrothermal rock–fluid systems, the experimental data are important in that they form a basis for evaluating a number of theories and hypotheses on the kinetics of water–rock interactions.
Section snippets
Experiments
Two batch experiments, with run times of 1872 h (78 days) and 120 h (5 days), involving perthitic alkali-feldspar dissolution in K-bearing (~ 0.20 KCl mol/kg) fluid at 200 °C, 300 bars were conducted at the University of Minnesota and National Energy Technology Laboratory (NETL), respectively. 40 g KCl solution and 1.5 g alkali-feldspar were used for both experiments. Prior to the experiments, the starting fluid was acidified to pH = 3.0 by addition of dilute HCl, so as to create initial
Cations, anions and dissolved SiO2
Time series changes in fluid chemistry from both experiments are listed in Table 2 and illustrated in Fig. 1. As anticipated from the relative abundances of fluid and mineral components used for the experiments, dissolved Cl− concentrations remained relatively constant. The concentration of dissolved K+, however, tended to decrease, although the extent of this represents a small fraction of that initially available in the fluid (200 mmol/kg).
Changes in dissolved concentrations of Na+, Ca2+, Al3+
Albite dissolution
Based on distribution of aqueous species calculations at experimental conditions, mineral saturation states during the experiments were determined (Table 4). The calculated saturation indices (SI, SI = log Q/K) indicate that throughout the experiments, the SI of albite is always negative, whereas the SI of K-feldspar becomes positive between 216 and 456 h of reaction (78-day experiment). Therefore, albite hydrolysis is predicted to occur throughout the experiment, while K-feldspar incrementally
Conclusions
Alkali-feldspar hydrolysis experiments using a well-mixed batch reactor allowed observations of time series in situ fluid chemistry at 200 °C and 300 bars to be integrated with the mineralogy and composition of reaction products retrieved after 5 and 78 days. Hydrolysis of the albite component of alkali-feldspar resulted in the formation of boehmite, and then kaolinite. SEM, HRTEM and XPS analyses of the surface of alkali-feldspar provide clear evidence for the preferential reaction of albite
Acknowledgments
Material in this paper is based upon work supported by the U.S. Department of Energy under Award No. DE-FG26-04NT42125 to CZ and WES and partially by the National Science Foundation under Award No.'s EAR0423971 and EAR0509775 to CZ. Any opinions, findings, and conclusions or recommendations expressed in this material, however, are those of the authors and do not necessarily reflect the views of the United States Government or any agency thereof. We thank Rick Haasch and John Baltrus for
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Present address: Department of Geology and Geophysics, University of Wisconsin-Madison, Madison, WI 53706, USA.